The reaction between nitric acid (HNO3) and barium carbonate (BaCO3) produces barium nitrate (Ba(NO3)2), water (H2O), and carbon dioxide (CO2). The balanced chemical equation is: 2HNO3(aq) + BaCO3(s) → Ba(NO3)2(aq) + H2O(l) + CO2(g).
This equation shows a 2:1 molar ratio between nitric acid and barium carbonate. For every two moles of nitric acid consumed, one mole of barium carbonate reacts. This ratio dictates the amount of products formed. For example, reacting 2 moles of HNO3 yields 1 mole of Ba(NO3)2, 1 mole of H2O, and 1 mole of CO2.
Calculating the theoretical yield of products requires knowing the limiting reactant. This is the reactant completely consumed first, determining the maximum amount of products possible. Identify the limiting reactant by comparing the molar ratio of reactants to the stoichiometric ratio in the balanced equation. The reactant with the smaller resulting ratio is the limiting reactant.
For instance, if you react 0.5 moles of HNO3 with 0.3 moles of BaCO3, HNO3 is limiting because (0.5 moles HNO3 / 2) < (0.3 moles baco3 / 1). The maximum yield of Ba(NO3)2 would be 0.25 moles (half the moles of the limiting reactant). This translates to grams using the molar mass of Ba(NO3)2 (261.34 g/mol).
Remember that the actual yield might be less than the theoretical yield due to factors like incomplete reactions or product loss. Percent yield, calculated by dividing the actual yield by the theoretical yield and multiplying by 100%, provides a measure of reaction efficiency.
